What is the pH at the equivalence point of a titration when 0.1000 mol L-1 HCI is used to titrate 20.00 mL of a 0.2502 mol L-1 methylamine, CH3NH2, solution? Kp(CH3NH2) = 4.4x10-4
Q: The next 9 questions are related to the titration of 40.00 mL of a 0.0900 M acetic acid solution…
A: The balanced equation for the given titration reaction is,
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Q: Question is attached
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Q: What is the pH at the equivalence point?
A: We have to find the pH of solution
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A: Given, Volume of acetic acid, HOAc = 20.00 mL = 0.02 L (1mL = 0.001 L) Molarity of acetic acid,…
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A: pH = pKa + log[C3H5O2-]/[HC3H5O2] Number of mol = Molarity x Volume (L)
Q: What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of…
A: Equivalence point is a point where just enough amount of titrant is added to neutralize the…
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A: Given [Mg(OH)2] = 3.2 × 10-4 M
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Q: In titrating 10 ml of 0.1N HA (pKa=4),the pH after the addition NaOH is O 2.32 3.25 O 3.61 4.50 4.36
A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid
Q: 4. Define equivalent point and end point in a titration between a strong acid and strong base.
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Q: For the titration of 20.0 mL of 0.150 M acetic acid (CH₂COOH, K₂ = 1.8x105) with 0.150 M NaOH, what…
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Q: A sample of acetic acid is titrated with a standardized NaOH solution. Before the end-point of tH…
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A: The equilibrium established in the reaction considered is, H+ + OCl-⇔HOCl
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Q: alculate the pH of a titration solution formed when 45.0 mL of 0.100 M NaOH is added to 50.0 mL of…
A: Given 45.0 mL of 0.100 M NaOH is added to50.0 mL of 0.100 M CH3COOH (Ka = 1.8×10-5). pH is to be…
Q: What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of…
A: Equivalence point is a specific state during neutralization at which all hydrogen ions are reacted…
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Q: The half-equivalence point of a titration occurs half way to the equivalence point, where half of…
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Q: #6 Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution…
A: Given, Volume of HCl = 40.00 mL = 0.040 L (1mL = 0.001 L) Molarity of HCl = 0.1000 M = 0.1000…
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Q: What is the pH of the solution that results from mixing 75 mL of 0.50 M NH 3(aq) and 75 mL of 0.50…
A: The solution is given below -
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- The molar solubility of the salt with generic formula AB2 is 3.26 × 10-5 M in pure water. Calculate the Ksp for this salt. Group of answer choices no correct answer 1.39x10-13 4.25x10-9 1.59x10-18 3.46x10-14One liter of a 0.1 M Tris buffer (pKa of Tris = 8.3) is prepared and adjusted to a pH of 2.0. B) What is the pH when 1.5 mL of 3.0 M HCl is added to 1.0 L of the buffer?Answer with 2 significant digits.A 50.0 mL sample of a 1.00×10-3 M solution of silver(I) nitrate is mixed with 50.0 mL of a 1.00×10-3M solution of potassium carbonate. A) Identify a possible precipitate: Answer B) What is the Qsp for this compound in the final solution?Express your answer to three significant figures. Qsp =Answer C) What can you say about the final solution? A table of Ksp values is available on ACORN under the Midterm 3 heading.
- A solution is 0.015 M in Ba(NO3)2 and 0.012 M in AgNO3. Solid sodium chromate(Na2CrO4) is slowly added without changing the volume of the solution.Ksp of Ag2CrO4 = 9.0×10-12 and Ksp of BaCrO4= 8.5×10-11(a) Which salt will precipitate first? Answer: __________________(b) What is the chromate concentration required to precipitate the salt named in part (a)?PLS ANSWER ASAP HUHU I ONLY HAVE 5 MINS LEFT.. THANKSS!! What is the molar solubility of AgI Ksp = 8.3 × 10-17 in the presence of 0.05 M KI? Group of answer choices 9.11 x 10^(-9) M 3.44 x 10^(-14) M 2.34 x 10^(-11) M 1.66 x 10^(-15) MConsider the equilibrium reaction: AX3(s) ⇌ A3+(aq) + 3X-(aq). What is the solubility of AX3 (MM = 78.0g/mol) in mg/L at 250C if its Ksp is 1.0 x 10−33? answer: 1.92x10-4 mg/L
- The value of Ksp for lead(II) chloride at a certain temperature is 1.55×10-5. Calculate the solubility of lead(II) chloride in a solution of 0.100 M sodium chloride. Express your answer to three significant figures. S = Answer mol L-How many grams of NaOH are needed to make 100.0 mL of a 0.130 M acetic acid/acetate buffer pH 5.20 from 1.00M acetic acid and solid NaOH? pka for acetic acid is 4.74 and molecular weight for NaOH is 40.00 g/mol I know the answer is 0.386 grams, please show workA 0.1057 N HCl solution was used to titrate a sample containing Ba(OH)2. If 35.78 mL of HCl was required to exactly react with 0.8772 g of the sample, what is the percent of Ba(OH)2 in the sample? 2HCl + Ba(OH)2 ? BaCl2 + 2H2O Answer = ______ %
- 1. A 0.1250-g sample of pure (100%) of K2Cr2O7 was dissolve in 250-mL volumetric flask, and dilute to volume, producing a concentration of 1.700 × 10-3 M. The resulting solution is an example of a standard solution prepared from a primary standard. Select one: a. True b. False 2. Which of the following is not an example of a standard solution? a. 1000 ppm Lead Nitrate solution b. 1.000g pure sodium carbonate dissolved in 1L of solution c. 3:4 nitric acid: hydrochloric acid solution d. NaOH solution standardized using KHP e. 0.104 M NaOHAnswer if true or false , if false, put the correct answer 1. There is 11.34 mmol in 0.2011 of 0.5604 M HgCl2 2. The x axis of sigmoidal titration curve is p function of the analyte or titrant 3.The concentration of the secondary standard is relative to a primary standard 4. There is 110 mmol in 79.8 mL of 0.1379 M NH4VO3 (116.98 g/mol)A 250.00 mL solution of 0.00215 M AB4 is added to a 230.00 mL solution of 0.00380 M C3D2. What is pQsp for A3D4? Answer: (18.607)